1. In the Deacon process for the manufacture of chlorine, HCl and O2 react to form...

1. In the Deacon process for the manufacture of chlorine, HCl and O2 react to form Cl2 and
H2O. Sufficient air (21 mole% O2, 79% N2) is fed to provide 35% excess oxygen, and the
fractional conversion of HCl is 85%.

(a) Calculate the mole fractions of the product stream components, using atomic species
balances in your calculations.

(b) Again calculate the mole fractions of the product stream components, only this time
use the extent of reaction in the calculations.

(c) An alternative to using air as the oxygen source would be to feed pure oxygen to
the reactor. Running with oxygen imposes a signi cant extra process cost relative to
running with air, but also offers the potential for considerable savings. Speculate on
what the cost and savings might be. What would determine which way the process
should be run?

Expert Solution

queen_honey_blossom answered 11 months ago

In the Deacon process for the manufacture of chlorine, HCl and O2 react to form Cl2...

In the Deacon process for the manufacture of chlorine, HCl and O2 react to form Cl2 and H2O. Sufficient air (21 mole % O2, 79% N2) is fed to provide 35.0% excess oxygen and the fractional conversion of HCl is 75.0%. a. Calculate the mole fractions of the product stream components using atomic species balances in your calculation. b. Again calculate the mole fractions of the product stream components using the extent of reaction and stoichiometric coefficients in the calculation...

1. Chlorine and fluorine gases can react to form chlorine trifluoride: Cl2(g) + 3F2(g) -->...

1. Chlorine and fluorine gases can react to form chlorine trifluoride: Cl2(g) + 3F2(g) --> 2ClF3(g) What is the theoretical yield in grams of chlorine trifluoride (ClF3)if a 2.0 L container at 350 K initially contains Cl2 gas at a partial pressure of 1.0 atm and fluorine gas at a partial pressure of 2.0 atm? Hint: This is a limiting reactant problem. A. 8.6 g ClF3 B. 21.5 g ClF3 C. 13 g ClF3 D. 19.3 g ClF3

1 Hydrogen and chlorine react to produce hydrogen chloride (HCl) as shown below. At equilibrium, the...

1 Hydrogen and chlorine react to produce hydrogen chloride (HCl) as shown below. At equilibrium, the flask contains 0.239 g of HCl, 0.254 g of Cl2 and 0.00013 g of H2. Calculate the value of Kc. The reaction is: H2 + Cl2 <--> 2HCl Hint: Work in mol/L. 1.72 x 103 5.4 x 10-2 1.84 x 102 3.55 x 10-5 2.99 x 104 2.If 40 g of HF are initially placed in an empty 1 L flask, calculate the amount of...

A 2.47×10-1 g sample of HCl and a 8.82 g sample of O2 react in a...

A 2.47×10-1 g sample of HCl and a 8.82 g sample of O2 react in a closed 2.25 L container at 487 K, according to the following balanced chemical equation: 4HCl(g) + O2(g) → 2H2O(l) + 2Cl2(g) Calculate the PCl2 (in atm) in the container after the reaction has gone to completion.

he Deacon process uses hydrochloric acid and oxygen from air to produce chlorine gas and water....

he Deacon process uses hydrochloric acid and oxygen from air to produce chlorine gas and water. Air is fed into the reactor at about 35% excess, and the fractional conversion to chlorine gas is about 85%. Procurement needs to know how much acid to purchase, and we are thinking about using 37% w/w HCl (12M), which has an overall density of 1.19kg/L. How many litres of this 37% w/w HCl should we purchase per week to get 100,000 litres (STP)...

#1. (2 pts) If 20.00 grams of KClO3 react, how many grams of O2 will form?...

#1. (2 pts) If 20.00 grams of KClO3 react, how many grams of O2 will form? 2 KClO3 -->2 KCl + 3 O2 #2. (4 pts) 2.80 g solid Al is mixed with excess Cl2(g) forming solid AlCl3. After the reaction is over 4.53 g AlCl3 is collected. Write the balanced reaction, determine the theoretical yield, calculate the percent yield. #3. (4 pts) 15.0 mL of 0.200 M AgNO3(aq) is mixed with 20.0mL of 0.100 M K2CrO4(aq). 0.350 g of...

4HCl(g) +O2(g) >>>> 2H2O(l) + 2Cl2(g) When 63.1g of HCl are allowed to react with 17.2g...

4HCl(g) +O2(g) >>>> 2H2O(l) + 2Cl2(g) When 63.1g of HCl are allowed to react with 17.2g of O2 41.5g of Cl2 are collected A.) determine the theoretical yield of Cl2 for the reaction B.) determine the precent yield for the reaction

QUESTION #1: Carbon monoxide and chlorine gas react to form phosgene: CO(g)+Cl2(g)⇌COCl2(g) Kp = 3.10 at...

QUESTION #1: Carbon monoxide and chlorine gas react to form phosgene: CO(g)+Cl2(g)⇌COCl2(g) Kp = 3.10 at 700 K If a reaction mixture initially contains 321 torr of CO and 157 torr of Cl2, what is the mole fraction of COCl2 when equilibrium is reached? QUESTION #2: Calculate the concentration of all species in a 0.150 M solution of H2CO3 [H2CO3], [HCO−3], [CO2−3], [H3O+], [OH−] = _____?_____ QUESTION #3: Write the formula for the conjugate base of each of the following...

Aqueous hydrochloric acid and aqueous potassium permanganate react to form chlorine gas, liquid water, solid potassium...

Aqueous hydrochloric acid and aqueous potassium permanganate react to form chlorine gas, liquid water, solid potassium chloride, and aqueous manganese chloride. If 8.88×104 milligrams of hydrochloric acid reacts with an excess of potassium permanganate, determine the mass of chlorine in grams. I really have no Idea how to approach this problem. Please help this is due at midnight tonight. A. 1.01×106 grams B. 7.79×103 grams C. 2.59×108 grams D. 5.53×105 grams E.54.0 grams

When 20.0 g C2H6 and 60.0 g O2 react to form CO2 and H2O, how many...

When 20.0 g C2H6 and 60.0 g O2 react to form CO2 and H2O, how many grams of water are formed?

Question